Which side of this proton transfer reaction is favored at equilibrium? Ö: HO: (Na* spectator ion is not shown.) OH Reactants (left side) Products (right side) Neither side is favored H₂O:
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
Not sure, its multiple choice so one answer only
![### Understanding Proton Transfer Reactions and Equilibrium
#### Question:
Which side of this proton transfer reaction is favored at equilibrium?
#### Chemical Reaction:
\[ \begin{array}{c}
\mathrm{CH_3(CH_2)_2COOH} + \mathrm{OH^-} \rightleftharpoons \mathrm{CH_3(CH_2)_2COO^-} + \mathrm{H_2O} \\
\end{array} \]
*Note: The \( \mathrm{Na^+} \) spectator ion is not shown.*
#### Options:
1. **Reactants (left side)**
2. **Products (right side)**
3. **Neither side is favored**
#### Explanation of the Reaction:
This is a proton transfer reaction. Here's a breakdown of the components:
1. **Reactants (left side):**
- **Propanoic acid (\( \mathrm{CH_3(CH_2)_2COOH} \))**: A carboxylic acid.
- **Hydroxide ion (\( \mathrm{OH^-} \))**: A strong base, typically derived from alkali.
2. **Equilibrium Arrows**: Indicate that the reaction can proceed in both forward and backward directions until equilibrium is established.
3. **Products (right side):**
- **Propanoate ion (\( \mathrm{CH_3(CH_2)_2COO^-} \))**: The conjugate base of the propanoic acid.
- **Water (\( \mathrm{H_2O} \))**: Formed by the protonation of the hydroxide ion.
#### Analyzing the Equilibrium:
- **Acid-Base Strengths**: The reaction equilibrium is influenced by the relative strengths of the acids and bases involved.
- **Propanoic acid** is a weak acid, whereas **hydroxide ion** is a strong base.
- **Water** is a weak acid when compared to the hydroxide ion.
- The equilibrium generally favors the formation of the weaker acid and base. Given that water is weaker (less likely to donate a proton) than propanoic acid, the equilibrium will likely shift towards the products.
#### Conclusion:
Hence, the side favored at equilibrium for this reaction is:
**[Products (right side)]**
By understanding the relative strengths of the acids and bases, one can determine](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ffb6abb0f-4367-447a-ab31-0a44cd95ae50%2Feccdbfd3-33ef-486b-98c0-9ff2ec0bc81a%2F8bcd825_processed.png&w=3840&q=75)
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